Review - Spring Chapter 10 Multiple Choice: circle the best answer
1.
22.4 liters of a gas at STP are equal to?
A)
1 gram
B)
6.02 1023 grams
C)
1 mole
D)
22.4 moles
2.
Pressure is created by gas particles
A)
Being dependent on one another.
B)
Being attracted to one another.
C)
Bouncing off of each other and objects.
D)
Being independent of one another.
3.
When a gas sample in a closed container has its pressure decreased by a factor of four, what happens to its volume?
A)
It decreases by a factor of 4.
B)
It increases by a factor of 4.
C)
It neither decreases nor increases.
D)
none of the above
4.
What happens to the pressure of a gas when its temperature decreases, all other factors being equal?
A)
The pressure increases.
B)
The pressure decreases.
C)
The pressure remains equal.
D)
B or C
5.
When gases react according to a balanced chemical equation, such as 2H2(g) + O2 (g) 2 H2O(g), what do the coefficients represent?
A)
the gas masses in grams that react
B)
the gas pressures in atm that react
C)
the gas volumes in liters that react
D)
none of the above
6.
When combined, what gas laws are simply called “the combined gas law?”
A)
Charles', Gay-Lussac's, and Avogadro's
B)
Boyle's, Avogrdro's, and Gay-Lussac's
C)
Boyle's, Charles', and Gay-Lussac's
D)
Avogadro's, Boyle's, and Charles'
7.
Based on the equation below, how much N2 is needed to make 2 liters of NO? O2(g) + N2(g) 2 NO(g)
A)
cannot tell from the information given
B)
1 liters
C)
2 liter
D)
3 liters
8.
Ptotal = P1 + P2 + P3 represents what gas law?
A)
Avogadro’s law
B)
The combined gas law
C)
Boyles law
D)
Dalton’s law of partial pressure
9.
In the ideal gas law, what is R?
A)
the gas constant, 8.021 L.atm/mol.K
B)
the universal gas constant, 0.082 L.atm/mol.K
C)
the gas constant, 8.314 L.atm/mol.K
D)
the universal gas constant, 8.314 L.atm/mol.K
10.
What are taggants?
A)
Micron-sized polymer chips embedded in explosives
B)
Materials that accelerate an explosion
C)
Materials that modify an explosion
D)
Small, non-explosive molecules in explosives
Problems: show all work in the space provided, circle the correct answer. Don’t forget units.
11.
What is the pressure if there are 0.62 moles of helium in a container that is 2.00 L, and at a temperature of 24.0oC?
12.
A gas at 34oC has a volume of 45 L. If its temperature is changed to 55oC, what is the new volume?
13.
What is the temperature of a 1.5 L container of hydrogen gas at 2.5 atm, if it is pressurized to 8.5 atm, at a volume of 3.4L and a temperature of 45.6oC.
14.
If nitrogen gas in a 8.0 L container at a pressure of 3.4 atm is compressed to 3.5 L, what is the resulting pressure?
15.
A gas evolved during the fermentation of sugar was collected at 22.5oC and 802 mmHg. After purification its volume was found to be 25.0 L. How many moles of gas were collected?
16.
I place 0.5 moles of N2 and some oxygen in a 40L container at a temperature of 350 oC. The total pressure of the container is 4 atm. What is the pressure exerted by the oxygen?
17.
A toy balloon has an internal pressure of 1.2 atm and a volume of 3.0 L. If the temperature where the balloon is released is 22o C, what will happen to the volume when the balloon rises to an altitude where the pressure is 0.55 atm and the temperature is –12o C?
18.
What volume in liters will 8.0 moles of neon occupy at STP?
Short answer/essay. Thoroughly answer each question.
19.
A. State the four parts of the Kinetic Molecular Theory.
B. Based on the Kinetic Molecular Theory, describe why gases are compressible.
20.
Read the statements below and state whether or not you agree or disagree with the statement. Use the kinetic theory to support your opinion. a.) Gases have no set volume b.) As volume increases temperature decreases
21.
In the case study, how did the officials find the person responsible for the explosion?
22.
Describe an everyday application of Boyle's Law (pressure and volume).
23.
What is STP? Be very detailed.
Chapter 9 Multiple Choice: choose the best answer.
1.
What did the prosecution claim Kenny Richey had stolen to start a fire?
A)
paint thinner
B)
propane and paint thinner
C)
gasoline and paint thinner
D)
lighter fluid
2.
The First Law of Thermodynamics also goes by another name—what is it?
A)
the law of conservation of energy
B)
the law of conservation of mass
C)
the law of conservation of phase
D)
the law of conservation of calories
3.
When two or more objects touch and reach the same temperature, this condition is called
A)
static equilibrium
B)
isotonic equilibrium
C)
dynamic equilibrium
D)
thermal equilibrium
4.
In the lab using a constant pressure calorimeter (the Styrofoam cups), how do you find the final temperature of the metal?
A)
You take the metal and either hold it in your hand or place it on the lab bench, and use a thermometer to get the best temperature.
B)
Take the final temperature of the water. Thermal equilibrium makes it equal to the final temperature of the metal
C)
Substract the final temperature of the water from the initial temperature of the boiling water and divide by the mass.
D)
It has something to with the q’s.
5.
When first using a cold pack, the directions say to squeeze the center until a popping noise is heard. This allows the reactants to mix. What type of reaction is occurring?
A)
Exothermic
B)
Poikiothermic
C)
Endothermic
D)
Ectothermic
6.
In the compound H2SO4, what is the oxidation number of S?
A)
+6
B)
0
C)
–2
D)
–4
7.
The oxidation number of hydrogen in both sides of the following reaction 2 C2H6 + 7 O2 4 CO2 + 6 H2O, are the same. What is that number?
A)
0
B)
+1
C)
–1
D)
There is not enough information to tell.
8.
What is the oxidation number of Li in the compound Li2S?
A)
+1
B)
–1
C)
+2
D)
–2
9.
In the following reaction, how does the oxidation number of Oxygen change: CH4 + 2 O2 CO2 + 2 H2O?
A)
It goes from 0 to +2.
B)
It goes from 0 to –2.
C)
It does not change.
D)
There is not enough information to tell.
10.
What do all exothermic reactions produce?
A)
heat
B)
light
C)
smoke
D)
fumes
11.
What physical change occurs at the melting point of a material?
A)
liquid becomes gas
B)
solid becomes gas
C)
liquid becomes solid
D)
solid becomes liquid
12.
How is specific heat defined?
A)
the amount of heat needed to raise 1 mole of material 1oF
B)
the amount of heat needed to raise 1 g of material 1oF
C)
the amount of heat needed to raise 1 mole of material 1oC
D)
the amount of heat needed to raise 1 g of material 1oC
13.
What intermolecular forces account for the much higher specific heat capacity of water than of metals?
A)
Induced dipoles
B)
Hydrogen bonding
C)
Ion-dipole
D)
None of the above
14.
The amount of energy required to convert a liquid to a gas is known as what?
A)
the heat of vaporization
B)
the heat of conversion
C)
the heat of gasification
D)
the heat of nebulization
15.
What is the SI unit of heat energy?
A)
the joule
B)
the calorie
C)
the coulomb
D)
the oC
Math: Show all work, circle your answer, and don’t forget units.
16.
When a 213.0 g sample of copper is raised in temperature from 22.0oC to 95.0oC, what amount of heat is produced? The specific heat of copper is 0.38 J/goC
17.
Find the mass of a piece of aluminum that is heated to 100oC before being immersed in a calorimeter with 300 g of water at 22.0oC. The temperature of the water rises to a temperature of 28.5oC. Specific heat of water = 4.184 J/goC and the specific heat of aluminum is 0.90 J/goC.
18.
What is the heat of combustion of ethanol in J/g if it is 10.0 Cal/g. (1cal = 4.184 J, 1Cal = 1000cal)
19.
Calculate the mass of kerosene needed to produce 12,455 J of energy if the heat of combustion for kerosene is 250 J/g.
Short answer/essay. Thoroughly answer each question.
20.
Draw and label the parts of the fire triangle. Explain the significance of the fire triangle.
21.
Why is the activation energy of a reaction important?
22.
What is the difference between flashover and backdraft? How can each be prevented?
23.
In your opinion, was Kenny Richey innocent or guilty? State two facts from the case supporting your opinion.
24.
What is the purpose of a calorimeter? Describe two types.
25.
A forest fire is giving off billowing white smoke, yet 50 miles away part of the same forest fire is sending up clouds of black smoke. What is the difference between the two fires?
26.
Explain the process by which petroleum is refined.
27.
Write a balanced chemical equation for the combustion of the following:
Ethane
C8H160
28.
In the equations below, identify the element that is reduced and the element that is oxidized.
CH4 + O2 → CO2 + H2O
K + H2O → KOH + H2
Chapter 7 – handed out in class due to diagrams Chapter 6 Multiple choice: circle the best answer.
1.
Attractive forces that exist between particles are called what?
A)
intermolecular forces
B)
intramolecular forces
C)
heteromolecular forces
D)
intravenous-molecular forces
2.
In our chapter scenario, what was the first indicator that something was wrong with the administering of pain medication?
A)
The narcotics locker was tampered with.
B)
Patients continued to complain of pain.
C)
Nurses reported lost pain medication.
D)
Syringes had been stolen.
3.
In what type of compounds is the dipole-dipole force present?
A)
compounds in which a dipole can be induced
B)
compounds with two dipoles directly aligned
C)
compounds that contain a permanent dipole
D)
compounds with no dipole
4.
Why are narcotics controlled substances?
A)
because of the potential for abuse of them
B)
because of their medicinal value
C)
because of their cost
D)
because of the difficulty of manufacture of them
5.
The interpretation of blood spatter involves what property of liquids?
A)
that liquids have unique densities
B)
that liquids form spherical droplets
C)
that liquid volume:surface area ratios are constant
D)
that liquid surface areas are constant
6.
How is an induced dipole created?
A)
by an electron positioning next to it
B)
by the presence of a dipole next to it
C)
by dipoles placed on both sides of it
D)
by an electron inversion near it
7.
London dispersion forces are considered to be what?
A)
strong intermolecular forces
B)
strong intramolecular forces
C)
weak intermolecular forces
D)
weak intramolecular forces
8.
To what is the positive region of a polar molecule attracted?
A)
a magnet
B)
the positive region of a neighboring molecule
C)
the negative region of a neighboring molecule
D)
to a non-polar molecule, thus inducing a dipole
9.
Which bond would have the greatest dipole?
A)
Si-H
B)
H-H
C)
O-H
D)
Br-H
10.
Which of the following would have no dipole?
A)
H-H
B)
H-F
C)
H-C
D)
H-Cl
11.
Which of the following will form hydrogen bonds?
A)
methanol, CH3OH
B)
water, H2O
C)
neither of the above
D)
both of the above
12.
How can vapor pressure of a liquid be increased?
A)
add a solute to the liquid
B)
decrease the kinetic energy of the material
C)
cool the material
D)
heat the material
13.
How does boiling an unknown sample of water allow you to determine if it is pure water or a solution? (you are at sealevel)
A)
In pure water, the b.p. should be below 100oC
B)
In pure water, the b.p. should be above 100oC.
C)
In a solution, the b.p. should be lower than 100oC.
D)
In a solution, the b.p. should be higher than 100oC.
14.
How is molality defined?
A)
moles of solute per kilograms of solution or solvent
B)
moles of solute per grams of solution or solvent
C)
moles of solute per liters of solution or solvent
D)
moles of solute per mililiters of solution or solvent
15.
What is the one factor upon which boiling point elevation depends?
A)
number of particles in solution
B)
size of particles in solution
C)
charges of particles in solution
D)
types of particles in solution
16.
What is occurring at the freezing point of a liquid?
A)
Some liquid phase molecules are slowing and becoming solid.
B)
Some of the solid molecules have enough energy to become liquid.
C)
both of the above
D)
neither of the above
17.
Which of the following should depress a freezing point the most if all have the same molality?
A)
NaCl
B)
Na2SO4
C)
KCl
D)
LiCl
18.
Which of the following is the proper order for the listed compounds, from least to greatest elevation of the boiling point of water, assuming the same molality?
A)
NaCl, FeCl3, MgCl2
B)
MgCl2, NaCl, FeCl3
C)
NaCl, MgCl2, FeCl3
D)
FeCl3, MgCl2, NaCl
19.
What is the process called when particles in a solution move from a region of high concentration in some random fashion to a region of lower concentration?
A)
dilution
B)
effusion
C)
diffusion
D)
osmosis
20.
Osmotic pressure prevents what?
A)
a net change in volume across a semi-permeable membrane
B)
a loss of solvent through a semi-permeable membrane
C)
a loss of solute particles through a semi-permeable membrane
D)
a net change in mass across a semi-permeable membrane
Math: Show all work and circle your answer. Do not forget units and watch significant figures. Kbp = 0.512oC/m and Kfp = -1.85oC/m
21.
What is the freezing point temperature of an aqueous solution made with 0.20 m KBr?
22.
What is the molality of a solution of 13.5g of CaS in 100 g of water?
23.
What is the boiling point of a 500g aqueous solution with 54.5g of C6H12O6?
24. What is the molality of an aqueous solution of KF if the freezing point is -4.5oC? Short answer/essay: Thoroughly answer each question.
25.
Define dipole – induced - dipole and ion-dipole? Explain how the two are similar and how they are different.
26.
What is the role of osmosis in a hypotonic solution?
27.
When a solute is added to a solvent, why does the freezing point decrease?
28.
Explain why intermolecular forces have an effect on the boiling/freezing point, and state of matter.
29.
Explain surface tension.
30.
Define and explain the difference between induced dipole and hydrogen bond.
Chapter 5 MULTIPLE CHOICE: circle the best answer
1.
Which would be more harmful, a weak acid or a strong acid?
A)
Both are equally harmful
B)
The strong acid
C)
The weak acid
D)
It depends on which strong acid is being used.
2.
An acid donates a _ and a base donates a __
A)
Metal ion, metal ion
B)
H+, OH+
C)
OH-, H-
D)
H+, OH-
3.
Why is a molecular compound like ethylene glycol soluble in water?
A)
Both are non-polar molecules.
B)
Both are polar molecules.
C)
Both are small molecules.
D)
Both are liquid-state molecules.
4.
In general, when an aqueous solution is heated, what happens to the solubility of ionic compounds within it?
A)
Solubility decreases.
B)
Solubility increases.
C)
Kinetic energy is added by the solute.
D)
Kinetic energy is removed by the solute.
5.
Identify the weak electrolyte.
A)
H2SO4
B)
HF
C)
HCl
D)
HNO3
6.
Why does powdered sugar dissolve in water more rapidly than a sugar cube?
A)
greater surface area of the powder
B)
more kinetic energy in the powdered sample
C)
greater concentration in the sugar cube
D)
greater density of the sugar cube
7.
A solution with a pH = 8.5 is said to be what?
A)
acidic
B)
basic
C)
neutral
D)
can't tell from the information given
8.
What is a strong electrolyte?
A)
a compound that completely forms ions in solution and conducts electricity
B)
a compound that only partially forms molecules in solution and conducts electricity
C)
a compound that completely forms molecules in solution and conducts electricity
D)
a compound that only partially forms ions in solution and conducts electricity
9.
Which compound could be an electrolyte?
A)
SO3
B)
NO2
C)
CH4
D)
MgCl2
10.
Of the group, SO2, SO3, and CO, which are non-electrolytes?
A)
SO2 and SO3 are non-electrolytes.
B)
SO2 and CO are non-electrolytes.
C)
All are non-electrolytes.
D)
All are electrolytes.
11.
What is a supersaturated solution?
A)
one that contains more than the maximum amount of solute that can be dissolved.
B)
one that contains less than the maximum amount of solvent that can be dissolved.
C)
one that contains the maximum amount of solution that can be dissolved.
D)
one that contains more than the maximum amount of a salt that can be dissolved.
12.
What kind of salt is NaCN?
A)
insoluble
B)
soluble
C)
sparingly soluble
D)
an insoluble solid
13.
The addition of KOH to HCl is what kind of reaction?
A)
a reduction–oxidation that does not make a precipitate
B)
a reduction–oxidation that makes a precipitate
C)
a neutralization that makes salt and water
D)
an addition that makes salt and water
14.
CaCO3 should be what, according to the solubility table?
A)
supersaturatable
B)
soluble
C)
insoluble
D)
molecular
15.
Saponification is?
A)
Grave wax
B)
A new type of reactions
C)
The reaction of NaOH with animal fat to make soap
D)
A new pH scale
16.
NaOH is classified as what kind of compound?
A)
weak base
B)
strong acid
C)
strong base
D)
weak acid
17.
CaS should behave how in water?
A)
It should be insoluble.
B)
It should be a molecular solid.
C)
It should be supersaturatable.
D)
It should be soluble.
18.
Which cation can make an insoluble product with Cl– in water?
A)
Na+
B)
Ag+
C)
Ca2+
D)
K+
19.
The pH scale
A)
Is a base 10 scale
B)
Goes from 0-14
C)
Was developed Soren Sorenson
D)
All of the above
E)
A and C only
20.
If the reaction AgNO3 + NaCl NaNO3 + AgCl were written out as a total ionic reaction, which ions would be the spectator ions?
A)
Ag+ and NO3–
B)
Na+ and Ag+
C)
Na+ and NO3–
D)
Cl– and NO3–
Math: Show all work. Circle your final answer.
21.
What is the molarity of a solution made from 0.25 moles of KBr and 0.80 L of water?
22.
A solution made from 19.0 g of NaBr and 1.5L of water has what molarity?
23.
If 300 mL of a 1.5 M solution is diluted to 750 mL, what is the molarity of the new solution?
24.
What is the [H+] concentration of a solution with a pH = 6?
25.
What is the pH of a solution with the [H+] = 2.4x10-6?
26.
The solubility of potassium cyanide is 50.0g/100mL. Would a solution of 22.5g/84mL be saturated, unsaturated, or supersaturated? (Show your math to support your answer)
Short answer/essay: thoroughly answer each question.
27.
Name the following acids and bases and identify as an acid or a base.
KOH _
b. HBr _
c. HNO3 _
28.
List two things that can increase the rate at which a substance is dissolved?
29.
Define electrolyte. Explain the relationship between a strong electrolyte, a weak electrolyte, a strong base and a weak base.
30.
Explain the purpose of a buffer, how one is made, and how it works..
31.
Predict the products and write the net ionic for the following: Silver nitrate + aluminum chloride →
32.
Give an example of a neutralization reaction.
33.
List three characteristics of an acid and three characteristics of a base.
34.
Explain why water is considered the universal solvent.
35.
Briefly explain why so many fish died in the White River near Anderson, Indiana.
36.
Use the graph below to answer the following questions.
Graph doesn't show up
a.
Identify the area that is supersaturated and the area that is saturated. (you may indicate your answer on the graph or describe the area below)
b.
What is the saturation point at 60oC?
c.
If the graph is the solubility curve for KNO3, name the solute and the solvent.
d.
At what temperature is the saturation point 80g/100mL?
Chapter 8 some diagrams will not show up Multiple choice: choose the best answer
1.
Which of the following happens with the valence bond theory?
A)
Electrons must not be shared.
B)
Orbitals must overlap.
C)
Orbitals must not overlap.
D)
Electrons must remain localized.
2.
What do the valence shells of all the noble gas elements have in common?
A)
a large size for its row on the periodic table
B)
a high ability to lose electrons
C)
a filled electron shell
D)
a high affinity for further electrons
3.
The correct Lewis dot structure for calcium is?
A)
B)
C)
D)
4.
Which is the correct Lewis dot structure for Germanium?
A)
B)
C)
D)
5.
How is ethane (C2H6) best represented by a Lewis structure?
A)
B)
C)
D)
6.
What does the double line, two lines on top of each other, represent in Lewis structures?
A)
A 6-electron triple bond
B)
A 4-electron double bond
C)
A 2-electron double bond
D)
A 4-electron triple bond
7.
What is the correct Lewis structure for methyl chloride, CClH3?
A)
B)
C)
D)
8.
What is wrong with this structure for gaseous hydrogen chloride: H – F?
A)
The lone pair electrons of hydrogen are not shown here.
B)
There are lone pair electrons on the fluorine which are not shown here.
C)
The bond between the two atoms should be a double bond.
D)
Nothing, the structure is correct.
9.
What is the best Lewis structure representation of formaldehyde, CH2O?
A)
B)
C)
D)
10.
A linear shaped molecule has what bond angle?
A)
180o
B)
109.5o 10
C)
120o
D)
90o
11.
What does valence shell electron pair repulsion theory help determine?
A)
atomic geometry
B)
molecular geometry
C)
molecular size
D)
atomic size
12.
What shape does carbon tetrabromide have?
A)
a triangular pyramid
B)
a square pyramid
C)
a square plane
D)
a tetrahedron
13.
Any molecule that has a central atom with no lone pairs, and three other, equivalent atoms connected to it, has what shape?
A)
square
B)
triangular
C)
tetrahedral
D)
trigonal planar
14.
Ionic bonds form through the
A)
Sharing of electrons
B)
Give and take of electrons
C)
Overlap of core electrons
D)
Giving away of valence and core electrons
15.
What trend do the noble gases display in relation to electronegativity?
A)
Electronegativity decreases as one goes down the noble gas column.
B)
Electronegativity increases as one goes down the noble gas column.
C)
The noble gases are all considered to have a electronegativity.
D)
For this column, there is no trend in electronegativity differences.
16.
How is the N–Br bond described?
A)
pure covalent
B)
polar covalent
C)
nonpolar covalent
D)
ionic
17.
What determines the charge an ion will have?
A)
Total number of electrons
B)
Valence electrons
C)
Number of valence electrons given away or received
D)
None of the above
18.
In what type of molecule is a resonance structure needed?
A)
Whenever a double bond can be positioned twice between two atoms with different electronegativities.
B)
Whenever a double bond can be positioned between two atoms with the same electronegativity.
C)
Whenever placement of a single bond can be in two positions that result in equivalent Lewis structures.
D)
Whenever placement of a double bond can be in two positions that result in equivalent Lewis structures.
19.
What is an antibody?
A)
A molecule specifically produced by the body to attack foreign antigens
B)
an antigen specifically produced by the body to attack foreign antigens
C)
a molecule specifically produced by the body to attack foreign antibiotics
D)
an antigen specifically produced by the body to attack foreign antibiotics
20.
VSEPR theory takes into account what two factors when determining molecular geometry?
A)
The location of lone pair valence electrons, plus the number of bonds.
B)
The size and location of lone pair valence electrons, plus the location of bonds.
C)
The location of lone pair valence electrons, and the location and number of bonds.
D)
The location of lone pair valence electrons, and the length of single and double bonds.
Short answer: thoroughly answer each question.
21.
What determines whether a compound will form an ionic or a covalent bond?
22.
What are resonant structures?
23.
What is wrong with the statement, “nonpolar molecules must always be composed of nonpolar bonds?”
24.
What are stereoisomers?
25.
Explain the function of neurotransmitters and by what means many illegal drugs affect the human brain.
26.
What is an immunoassay?
27.
Draw the Lewis Structure for MgF2
28.
Ionic bonds are known as the stronger bond. Explain this statement.
29.
What are valence electrons and how do you obtain this information from the periodic table?
30.
Draw the Lewis Structure for dihydrogen monosulfide.
31. Explain the scientific reason that allowed Christina Martin to have a second trial?
32. Complete the chart below:
Chapter 10
Multiple Choice: circle the best answer
2H2(g) + O2 (g) 2 H2O(g), what do the coefficients represent?
O2(g) + N2(g) 2 NO(g)
Problems: show all work in the space provided, circle the correct answer. Don’t forget units.
15.
Short answer/essay. Thoroughly answer each question.
B. Based on the Kinetic Molecular Theory, describe why gases are compressible.
a.) Gases have no set volume
b.) As volume increases temperature decreases
Chapter 9
Multiple Choice: choose the best answer.
2 C2H6 + 7 O2 4 CO2 + 6 H2O, are the same. What is that number?
CH4 + 2 O2 CO2 + 2 H2O?
Math: Show all work, circle your answer, and don’t forget units.
1Cal = 1000cal)
Short answer/essay. Thoroughly answer each question.
Chapter 7 – handed out in class due to diagrams
Chapter 6
Multiple choice: circle the best answer.
Math: Show all work and circle your answer. Do not forget units and watch significant figures.
Kbp = 0.512oC/m and Kfp = -1.85oC/m
24. What is the molality of an aqueous solution of KF if the freezing point is -4.5oC?
Short answer/essay: Thoroughly answer each question.
Chapter 5
MULTIPLE CHOICE: circle the best answer
Math: Show all work. Circle your final answer.
Short answer/essay: thoroughly answer each question.
Silver nitrate + aluminum chloride →
Graph doesn't show up
Chapter 8 some diagrams will not show up
Multiple choice: choose the best answer
10
Short answer: thoroughly answer each question.
31. Explain the scientific reason that allowed Christina Martin to have a second trial?
32. Complete the chart below: